How Does Adding KSCN Affect Fe3+, SCN-, and FeSCN2+ Concentrations?

In summary: So the concentration of Fe3+ and FeSCN2+ would decrease while the concentration of SCN- would increase. The iron concentration would not remain constant because it is not a part of the reaction being manipulated. The kind of shift involved would be a shift to the left, towards the reactants.In summary, the experiment tested Le Chatelier's Principle by diluting a stock solution of FeSCN-(aq) with water and adding KSCN to one test tube. The concentration of Fe3+(aq) and FeSCN2+(aq) decreased while the concentration of SCN-(aq) increased when KSCN was added. The iron concentration did not remain constant as it was not part of the reaction being manipulated.
  • #1
Veronica_Oles
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Homework Statement


During class we did a lab testing Le Chatelier's Principle where we took FeSCN-(aq) and added water in order to dilute it to a lighter colour (red to orange) and to make a stock solution. We then divided the stock solution into several test tubes. In one of them we added KSCN.

The question asked is:

How does the concentration of Fe3+(aq), SCN-(aq) and FeSCN2+(aq) change if the KSCN is added to the test? What remains constant? What kind of shift is involved?

Homework Equations

The Attempt at a Solution



I just need clarification to see if I'm doing this correctly. When we add KSCN to a test tube with the stock solution the solution went from orange to yellow. When it asks about how the concentration changes, it changes because there is more KSCN added. Meaning there will be more SCN-(aq), would this be correct? Pertaining to the question what remains constant would that just simply be the iron? And lastly what kind of shift involved would be a shift to the left because it favors the reactants.
 
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  • #2
Veronica_Oles said:
Pertaining to the question what remains constant would that just simply be the iron?

You have changed the total volume, how can the iron concentration remain constant?

I can be wrong, but at a first sight looks like the experiment is a bit misleading. Color change is most likely effect of dilution, not of a shift in the reaction.
 
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  • #3
Borek said:
You have changed the total volume, how can the iron concentration remain constant?

I can be wrong, but at a first sight looks like the experiment is a bit misleading. Color change is most likely effect of dilution, not of a shift in the reaction.
Oh okay that makes sense
 

FAQ: How Does Adding KSCN Affect Fe3+, SCN-, and FeSCN2+ Concentrations?

What is Le Chatelier's Principle?

Le Chatelier's Principle is a principle in chemistry that states that when a system at equilibrium is subjected to a stress or change, the system will adjust in a way to minimize the stress or change and maintain equilibrium.

How do you test Le Chatelier's Principle?

To test Le Chatelier's Principle, you can perform a series of experiments where you manipulate a system at equilibrium and observe the changes in the equilibrium position. This can be done by changing the concentration, pressure, or temperature of the system and observing the resulting shift in equilibrium.

What is an example of testing Le Chatelier's Principle?

An example of testing Le Chatelier's Principle is adding more reactants to a chemical reaction at equilibrium and observing the resulting shift in equilibrium towards the products to minimize the increase in concentration of the reactants.

Why is it important to test Le Chatelier's Principle?

Testing Le Chatelier's Principle is important because it helps us understand how different factors such as concentration, pressure, and temperature affect the equilibrium of a system. This knowledge is crucial in predicting and controlling the outcomes of chemical reactions.

What are the limitations of testing Le Chatelier's Principle?

One limitation of testing Le Chatelier's Principle is that it only applies to reversible reactions at equilibrium. It does not apply to irreversible reactions or reactions that are not at equilibrium. Additionally, the principle does not provide information on the rate of the reaction, only on the position of equilibrium.

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